Acids and Bases key terms

alkaline
the solution formed when a base completley dissociates in water to yield aqueous OH- ions
arrhenius acid
a chemical compound that increases the concentration of hydrogen ions, H+, in aqueous solutions
arrhenius base
a substance that increases the concentration of hydroxide ions, OH-, in aqueous solutions
binary acid
an acid that contains only two different elements: hydrogen and one of the more electronegtive elements
oxyacid
an acid that is a compound of hydrogen, oxygen, and a third element, usually a nonmetal
strong acid
one that ionizes completley in aqueous solutions
weak acids
acids that are weak electrolytes
amphoteric
any species that can react as either an acid or a base
Bronsted-Lowry acid
is a molecule or ion that is a proton donor
Bronsted-Lowry Base
is a molecule or ion that is a proton acceptor
Bronsted-Lowry Acid-base reactions
protons are transferred from one reactant (the acid) to another (the base)
monoprotic acid
an acid that can donate only one proton (hydrogen ion) per molecule
polyprotic acid
ana tom that can donate more than one proton per molecule
diprotic acid
can donate two protons per molecule
triprotic acid
an acid able to donate three protons per molecule
Lewis acid
an atom, ion, or molecule that accepts an electron pair to form a covalent bond
Lewis base
an atom, ion, or molecule that donates an electron pair to form a covalent bond
Lewis acid-base reaction
the formation of one or more covalent bonds between an electron-pair donor and electron pair acceptor
conjugate base
the species left after a Bronsted-Lowry acid has given up a proton
Conjugate acid
species left after a Bronsted-Lowry base gains a proton
neutralization
the reaction of hydronium ions and hyroxide ions to form water molecules
salt
ionic compound composed of a cation rom a base and an anion from an acid

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